The Universe and the universal laws of physics, thermodynamics, gravity and matter have all been well established for more than 13 billion yrs. Only 5 billion yrs. ago, in our Milky Way Galaxy of 400 billion stars, a benign cloud containing 90% of Hydrogen, combined with clouds containing 10% of other Nobel gases. The gases were interlaced according to their atomic weights as they, merged and began to drift. The formed gases drifted into an enormous amount of intrinsic electrically charged fissile atoms of naturally occurring galactic elements, integrating with the gases and combining. As the cloud drifted through an absolute zero region of the galaxy, its incorporated gases froze into gigantic, towering mountains of a combination of galactic mixed gases and elements. Embedded in the frozen gas cloud were also some extremely hot, cloud consuming ions. A fusion process was set into motion when friction from the charged galactic ions, ignited and began to consume the flammable gas cloud. The ignited gases, fused a hot spot which, then rendered liquid molten from the galactic elements. The impurities from the solid elements in the hot spot, formed into a slag cauldron which then began to heat up and thaw our frozen young star 4.9 billion yrs. ago. The frozen gas mountains thawed and breached the ruptured surface of our new Sun, flowing toward and finally reaching the extremely hot cauldron, with a mixture of liquefied homogenous gases.
When the thawed, liquefied gases made contact with the molten elements, a cataclysmic molten "splash", gas atomic explosion resulted within the enclosed cauldron (Galvani's Law).
The combination of ionic energy from fission and galvanic/ gas steam pressure produced from fusion caused the firstinternal solar eruption from atomic energy. The tremendous heat and pressure from the first powerful internal explosion caused the thawed, extremely hot neutrons of the fissionable atoms to melt. In that extreme environment the atoms were stripped bare of their neutrons, to a state of unstable ionized and un-ionized electrons (-) and protons (+). A Fission process began from the extreme heat, which caused the bare nuclei to collide and produce enough energy to split and separate the atoms into their sub-atomic state of quarks, neutrinos and leptons (Pauli's Exclusion Principle). The tremendous internal atomic explosion with the force of an exploding star ejected the mountains of thawed unstable sub-atomic photosphere and gases upward with extreme pressure and force within a confined area of the cauldron. The tremendous pressure from the first internal atomic explosion, blasted the small lighter atoms of Hydrogen and other sub-atomic Noble gases into the larger, heavier Oxygen, Etc. atoms. The explosion pierced and impregnated the unstable Oxygen atoms, with the propelled Hydrogen atoms, combining and altering the sub-atomic Noble gases for the first time. This amalgamating and incorporating of sub-atomic ions under extreme heat and pressure began the natural process of the formation of water and other compounds. The process continued, when the impregnated Oxygen atoms were exploded into the absolute zero temperature of interstellar space under extreme atomic pressure from within the confined cauldron of the hot spot. When the encapsulated Hydrogen atoms were blasted into the absolute zero environment, they bonded forever with the Oxygen atoms and became one compound atom with a ratio of 2H:1O, for the first time ever. The extreme pressure and temperatures permanently bonded and compounded the atoms of H.,O.,C.,N.,and etc. into their present, compounded state of H2O (water) and other compounded atoms e.g. CO2, N2+O2,etc. The first eruption simultaneously forged the Kuiper Belt, extending it out 50 AU from the Sun. It also established The Oort (Hydrogen) Cloud which our Sun uses as its fuel source. The first eruption also and simultaneously defined the boundaries of our Heliosphere more than 4.8 billion yrs. ago.
When you increase the temperature the solubility of a solute in a solution increases. This is due to the fact that heat is required to break the bonds that are holding the molecules in the solid together. Note that the opposite is true for gases, though.
Solubility is the ability of a substance (solute) to make a solution with another substance (solvent). The solvent is usually a liquid, and the solute can be a solid, liquid, or gas. The solute is usually dissolved into the liquid to create the solution.
most liquids hold less gasses as they heat up. Water being an exception as it nears freezing. Thus ice floats.
it decreases solubility.... by damion /\
carbonation is the most common form of dissolving a gas into a liquid. gasses are much more soluble into liquids ant high pressure
Pressure can affect the solubility but the effect is not important.
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Type your answer here... tamprature and concerntration..
If the pressure of the gas increase, the solubility in a liquid increase.
Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. This means that as the pressure of the gas increases, the solubility of the gas in the liquid also increases. By knowing the partial pressure of the gas and the Henry's Law constant for that specific gas and liquid, one can calculate the solubility of the gas in the liquid.
Increasing temperature decreases gas solubility in water due to reduced gas solubility at higher temperatures. In contrast, increasing pressure increases gas solubility in water according to Henry's law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid.
Increasing temperature decreases the solubility of a gas solute in a liquid solvent. This is because higher temperatures increase the kinetic energy of molecules, leading to weaker gas-liquid interactions and reduced solubility.
More gas dissolves into the liquid.
The amount of gas that will dissolve in blood plasma or any other liquid is determined by the partial pressure of the gas above the liquid and the solubility of the gas in that particular liquid. According to Henry's law, the concentration of the gas dissolved in a liquid is directly proportional to the partial pressure of that gas above the liquid.
Factors that determine how much of a gas can dissolve in a liquid include the partial pressure of the gas, temperature, and the chemical nature of both the gas and the liquid. Generally, higher pressure, lower temperature, and a stronger attraction between the gas and the liquid can all increase the solubility of the gas in the liquid.
If you are talking about the solubility of gasses in a liquid then lowering the temperature will increase the solubility of the gas
I'm not 100% sure that "solubility" is the right word to use here, but the amount of dissolved gas in a liquid will decrease as the partial pressure of the gas above the liquid decreases.Basically The solubility decreases.